Considering the definition of STP conditions, the correct answer is option D. 22.01 grams of CO₂ will ocupy at STP 11.35 L.
The STP conditions refer to the standard temperature and pressure. Pressure values at 1 atmosphere and temperature at 0 ° C are used and are reference values for gases. And in these conditions 1 mole of any gas occupies an approximate volume of 22.4 liters.
On the other side, the molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
In this case, you have 11.35 L of CO₂. The molar mass es 44.01 [tex]\frac{g}{mole}[/tex].
Next, you can apply the following rule of three: If by definition of STP conditions, 22.4 L are contained in 1 mole, 11.35 L are contained in how many moles?
[tex]number of moles=\frac{11.35 Lx1 mole}{22.4 L}[/tex]
number of moles= 0.5 moles
Now, you can apply the following rule of three: If by definition of molar mass 1 mole of carbon dioxide contains 44.01 grams, 0.507 moles of the compound contains how much mass?
[tex]mass=\frac{0.5 molesx44.01 grams}{1 mole}[/tex]
mass= 22.005 grams≅ 22.01 grams
Finally, the correct answer is option D. 22.01 grams of CO₂ will ocupy at STP 11.35 L.
Learn more about STP conditions:
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